Question

Using Le Chatelier’s principle, predict which equilibrium system below decrease the concentration of the reactant (H2CO3) as a result of the stress (change) added to the system.

The reaction being studied is: H2CO3(aq) H+(aq) + HCO3-(aq)

a. decrease H+ concentration by adding NaOH.
b. a catalyst is added.
c. Add more HCO3- by adding NaHCO3(s)

Answer 1

decrease H+ concentration by adding NaOH.

Step-by-step explanation:

H2CO3→ H+ + HCO3-

A decrease in H^+ concentration will lead to a decrease of the H2CO3 concentration since more of it will now dissociate to the bicarbonate ion (equilibrium position shifts towards the right). This is because as equilibrium position shifts towards the right as the hydrogen ions are removed it decreases the concentration of the carbonic acid in the system as shown by the equation above.

Answer 2

The correct answer is c add more HCO3- by adding NaHCO3.

Step-by-step explanation:

The reaction mentioned in the question is carried out by bicarbonate buffer system of our body to maintain the normal acid base balance.

Now concentration of the reactant (H2C03) is decreased then NaHCO3 should be added which undergo breakdown to release bicarbonate ions(HCO3-).

The released bicarbonate ions then reacts with H+ to form Carbonic acid(H2CO3).Thus homeostasis of H2CO3 is maintained.